The depletion of ozone (O3) in the stratosphere has been a matter of great conce

Question

The depletion of ozone (O3) in the stratosphere has been a matter of great concern among scientists in recent years. It is believed that ozone can react with nitric oxide (NO) that is discharged from the high-altitude jet plane, the SST. The reaction is 0_3 + NO = 0_2 + N0_2 If 0.815 g of O3 reacts with 0.691 g of NO, how many grams of N02 will be produced? gNQ2 Which compound is the limiting reagent? nitric oxide (NO) ozone (O3) Calculate the number of moles of the excess reagent remaining at the end of the reaction, mol

Explanation / Answer

The reaction is: O3 + NO O2 + NO2

From the reaction is clear that 48 g of O3 reacts with 30 g of NO gives 46 g of NO2.

0.815 g of O3 needs (0.815 x 30)/48 = 0.509 g NO. But we have 0.691 g of NO. That is NO is in excess, therefore O3 is the limiting reagent.

NO2 produced when 0.815 g of O3 reacts, will be: (0.815 x 46)/48 = 0.781 g

At the end of the reaction, the amount of excess reagent remains will be: 0.691 – 0.509 = 0 .182 g

Therefore the number of moles of the excess reagent remaining at the end of the reaction is:

0.182/30 = 0.00606 moles.

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